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d1i1m1o1n [39]
2 years ago
6

Calculate how many grams of the product form when 16.7 g of calcium metal completely reacts. Assume that there is more than enou

gh of the chlorine gas.
Ca(s) + Cl2(g) → CaCl2(s)
Chemistry
1 answer:
swat322 years ago
4 0

39.96 g product form when 16.7 g of calcium metal completely reacts.

<h3>What is the stoichiometric process?</h3>

Stoichiometry is a section of chemistry that involves using relationships between reactants and/or products in a chemical reaction to determine desired quantitative data.

Equation:

Ca(s) + Cl_2(g) → CaCl_2(s)

In this case, for the undergoing reaction, we can compute the grams of the formed calcium chloride by noticing the 1:1 molar ratio between calcium and it (stoichiometric coefficients) and using their molar mass of 40 g/mol and 111 g/mol by using the following stoichiometric process:

m_{ca_C_l_2}= 16.7 g Ca x \frac{1 mol \;of \;Ca}{40g Ca} x \frac{1 mol \;of \;CaCl_2}{1 mol \;Ca} x \frac{111g of \;CaCl_2}{1 mol \;CaCl_2}

m_{ca_C_l_2} = 39.96 g

Hence, 39.96 g product form when 16.7 g of calcium metal completely reacts.

Learn more about the stoichiometric process here:

brainly.com/question/15047541

#SPJ1

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